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प्रश्न
Give a reason for Ionisation potential increases across a period, from left to right
उत्तर
From left to right in the periodic table, atomic size decreases smaller the size more the effective nuclear charge. Therefore more energy is required to remove an electron from the atom, therefore, ionization potential increases.
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संबंधित प्रश्न
State the trends in ionization energy across the period.
Name the periodic property which relates to the amount of energy required to remove an electron from an isolated gaseous atom.
Li, K, Na, H (In the decreasing order of their ionization potential)
A, B, C are three elements in which B is an inert gas other than helium.With this information complete the following table.
| Element | Atomic number | No. of electrons in the valence shell | Group to which the element belongs |
| A | Z - 1 | ||
| B | Z | ||
| C | Z + 1 |
Also, explain the following : Ionization energy of element C is less than that of element A.
Choose the correct answer from the choice given:
Ionisation potential increases over a period from left to right because the
The changes in the properties of elements on moving from left to right across a period of the Periodic Table. For the property, choose the correct answer.
The ionization potential:
Arrange the following as per the instruction given in the bracket:
Potassium, Lithium, Sodium (increasing order of ionization potential).
Arrange the following as per instruction given in the bracket.
Li, K, Na, H (decreasing order of their potential ionisation)
Arrange the following in order of increasing ionisation energy:
P, Na, Cl
Explain your choice.
Ionisation Potential values depend on atomic size. Explain.
